AP EAMCET · Chemistry · Electrochemistry
The time required (in hours) to reduce \(3 \mathrm{~mol} \mathrm{of}\) \(\mathrm{Fe}^{3+}\) ions to \(\mathrm{Fe}^{2+}\) ions with 2.0 amperes of current is \(\left(1 \mathrm{~F}=96500 \mathrm{C} \mathrm{mol}^{-1}\right)\)
- A 30.2
- B 40.2
- C 10.2
- D 15.2
Answer & Solution
Correct Answer
(B) 40.2
Step-by-step Solution
Detailed explanation
\(\mathrm{i}=2.0 \mathrm{~A}, \mathrm{t}=?\) \(3 \mathrm{Fe}^{3+}+3 \mathrm{e}^{-} \rightarrow 3 \mathrm{Fe}^{2+}\) Charge of 3 moles of \(\mathrm{e}^{-}=3 \times 96500=289,500 \mathrm{C}\).…
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